Chem syllabus PDF

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chem syllabus for Tyler Maxwell's Fall 2019 course (CHM 2045) ...

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Syllabus CHM 2045C.0001 # 81486 Chemistry Fundamentals I Fall 2019 9:30 – 10:20 AM MWF VAB-132 Instructor: Dr. Tyler Maxwell Office: R1 244 Office Hours: Mon, Wed, Fri 10:30 – 12:00 PM

[email protected]

Text: Tro, Nivaldo. Chemistry A Molecular Approach, Pearson, 4th Edition, 2016. ISBN: 9781323769492 loose-leaf format with Mastering Chemistry and eBook at UCF bookstore. Hard cover and eBook formats are also available. A previous edition used book is also acceptable. We will not use Mastering Chemistry for a grade. To enhance your learning experience and provide affordable access to the right course material, this course is part of an inclusive access model called First Day™. You can easily access the required materials for this course at a discounted price, and benefit from single sign-on access with no codes required in UCF Webcourses. UCF Student Account Office will bill you at the discounted price as a course charge for this course. This charge will be posted to your account on September 3, 2019 for Fall 2019. It is recommended that you Opt-In as these materials are required to complete the course. You can choose to Opt-In on the first day of class, right within UCF Websourses. Be sure to Opt-In before the deadline of Saturday, August 31, 2019 at 11:59pm for Fall 2019 courses to have access to your course materials at the discounted price. Course goal: To provide you with an understanding of the basic chemical theory of atomic structure, chemical periodicity, stoichiometry, chemical reactivity, energy in chemical reactions, atomic structure, chemical bonding, and gases and their properties. Topics to be covered: The topics to be covered in this course will include, but not be restricted to, the scientific method, measurement, classification of matter, atomic structure, the Periodic Table, molecules, ions and their compounds, stoichiometry, solution chemistry, electrolytes, precipitation reactions, redox reactions, acids and bases, titration, energy and chemical reactions, calorimetry and Hess’s Law, quantum chemistry, atomic structure, the chemical periodicity, bonding and molecular structure, VSEPR theory, polarity, Valence Bond Theory, Molecular Orbital theory, gases and their properties. Learning Outcomes for CHM 2045C at Curriculum Alignment Matter, Measurement and Problem Solving Students will: - Understand the scientific method, classification of matter and chemical/physical changes. - become familiar with metric units and successfully navigate complex dimensional analysis problems - Calculate density and use it in applications such as identification of unknowns. - Apply concepts of accuracy and precision to determination of significant digits. Atoms and Elements

Students will - Learn the tenets of Dalton’s atomic theory, Law of Multiple Proportions and Law of Definite Proportions to explain atoms and molecules. - visualize the iterations of atomic structure through experiments including Thompson’s Cathode Ray Tube, Milliken’s Oil Drop experiment, and Rutherford’s gold foil experiment. - Describe the subatomic particles, properties and behavior and use them to identify elements, isotopes, ions, mass number and atomic number. - Us e the periodic table to predict reactivity and ions - Calculate weighted average atomic mass, molar mass and the number of atoms in a given mass of an element. Molecules, Compounds and Chemical Equations Students will - Be introduced to ionic and covalent bonds, distinguishing between molecular and ionic compounds. - Write formulas and names for ionic compounds and elucidate the charges of the ions. - Name and provide chemical formulas for binary molecular compounds and acids. - Use atomic mass to calculate formula mass and molar mass of compounds. - Calculate percent composition and, using elemental analysis, determine empirical and molecular formulas from mass % composition. - Balance chemical equations. Chemical Quantities and Aqueous Reactions Students will -Use stoichiometry to calculate theoretical yield, limiting and excess reagents, and percent yield. - Calculate molar concentrations and use the dilution formula. - Use molar concentrations to solve solutions stoichiometry problesm. - Identify electrolytes and nonelectrolytes, and identify the solubility of ionic compounds. -Use oxidation numbers to identify oxidation-reduction reactions and report the oxidizing and reducing agents in such reactions. -Identify acids and bases using Bronsted-Lowry and Arrhenius definitions and calculate the endpoint of a titration using solution stoichiometry. -Predict products for common gas-forming reactions. Gases Students will -Understand concepts of pressure and kinetic molecular theory of gases. - Utilize Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, Avogadro’s Law, the combined gas law and the ideal gas law. - Calculate densities of gases. - Explain the origin of the “absolute zero,” concept in terms of an ideal gas thermometer. - Measure pressure using a manometer. -Convert between commonly used units for pressure and volume.

- Distinguish between effusion and diffusion of gases, calculating root-meansquare velocities of gases and relative rates of effusion. - Understand deviations from ideality in gases and identify conditions that result in real gas behavior, and their resulting changes in molar volume and pressure. Understand the components of the Van der Waals equation for real gases. Thermochemistry Students will - Distinguish between potential and kinetic energy - Summarize the 1st Law of Thermodynamics, understanding state functions and heat and work. - Evaluate the difference between the system and surroundings and the sign of heat and work. - Use knowledge of bomb calorimeters to calculate internal energy under constant volume conditions, and coffee-cup calorimeters to calculate enthalpy under constant pressure conditions. - Use Hess’ Law to calculate heat of a reaction as a combination of other reactions. - Use heat of formation reactions to calculate reaction enthalpy. The Quantum Mechanical Model for the Atom Students will -Understand the properties of light, including diffraction and interference, and use dispersion relations to calculate wavelength, frequency, and energy of light. - Distinguish between the wave-nature and particle nature of the electron, citing examples from the photoelectric effect and the double slit diffraction. - Use the de Broglie relation to relate wavelength of light to momentum of particles. - Interpret the Bohr model of the atom utilizing concepts of atomic emission spectra and calculate the wavelength of light emitted from a Hydrogen atom using the Rydberg equation. - Describe shapes of molecular orbitals that arise from probability distribution of wavefunctions. - Use quantum numbers to describe orbitals occupied by electrons. Periodic Properties of Elements Students will - Use the aufbau principle and Hund’s rule to draw orbital diagrams and electron configurations. - Distinguish between valence electrons and core electrons, calculating effective nuclear charge and utilizing this concept to describe periodic trends in atomic radius, ionization energy, and electron affinity. Chemical Bonding: the Lewis Model Students will - Learn to represent valence electrons as dots and predict ionic compound structure using Lewis Theory. - Predict structures for atoms, isomers, and resonance structures. - Use electronegativity to predict bond polarity.

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Use formal charge to predict dominant resonance structures. Identify and justify exceptions to the octet rule. Use bond energies to calculate reaction enthalpy.

Chemical Bonding – Molecular Shapes, Hybridization and Molecular Orbital Theory Students will - Use VSEPR to predict molecular and electron group geometry. - Use VSEPR to predict bond angles - Use VSEPR to predict polarity of molecules. - Describe bonds in terms of orbital overlap and identify hybridization, sigma and pi bonds in hybrid orbital bond theory. - Use molecular orbitals to calculate bond order and predict para- and diamagentism of molecules.

Additional Learning Outcomes -Apply fundamental chemistry concepts to explain real-world phenomena. - Utilize chemical equations to make evaluations of potential fuels. - Understand how stoichiometry provides insight into carbon emissions and acid rain. - Utilize graphing software to perform graphical analysis. - Make measurements to understand the origin of significant figures and explain sources of error. - Learn the structure and language of technical reports and generate lab reports. -Begin to establish familiarity with peer-reviewed chemical literature. Discussion sessions: This course has eight discussions sessions, 50 minutes each, every week. You should be registered in one of them. Four sessions of Supplemental Instruction (SI) will be provided for this course. Grading: All exams, except the final, will be given during regularly scheduled class time. Your grade will be calculated on the basis of a percentage of total points. There will be no curve and grades will be assigned based on: 90-100 % = A; 80-89% = B; 70-79% = C; 60-69% = NC; < 60% = F. NC means No Credit. NC grade does not count toward your GPA. It affects your Financial Aid, though. In the event that you are absent for an exam, the percentage score from your final exam will be substituted for the missed exam. The percentage grade from your final exam will replace your lowest exam grade (if higher) if you have no missed exams. Exams will be 50 minutes each, with 20 questions, and will be worth 100 points each. The final exam will have 50 questions(*) and will last 2 hrs 50 minutes. All exams will be cumulative, mandatory, and computer-graded multiple choice format. Exam questions will be worked out in detail and posted by my office (CH 107A). Eight fifteen-minute quizzes will be given during the semester. They will be given in the discussion sections, with due notice. Quizzes will be worth 25 points each. Your best seven (7) quizzes out of nine (8) will be counted. The two lowest will be dropped. Students who leave the classroom after taking a quiz/exam will earn ZERO in such a test. (*) 40 Questions of the ACS standardized test will be part of the final exam. ALEKS: (Assessment and Learning in Knowledge Spaces) is a powerful, artificial-intelligence based teaching tool that we will be using to increase your chances of success in CHM 2045C. You will be required to complete objectives in ALEKS every week. You will first need to take an initial knowledge check so that

ALEKS can tailor a study plan that works for you, based on your current knowledge of chemistry. Take this initial knowledge check ASAP, so you have plenty of time to do any needed work. Attendance will be taken by means of Learning CatalyticsTM pop quizzes and will count toward your final grade. Grading Summary 4 Exams @ 100 points each Final exam Best 7 quizzes ALEKS Learning Catalytics/Attendance Total

400 points 200 points 175 points 105 points 20 points 900 points

A student ID will be required for each exam. Scientific non graphing calculators will be needed for the quizzes, exams and the final. Any use of electronic device (iPod, cell phone, MP3 player, laptop, tablet…) during classes and exams is strictly prohibited. Any use of such device will be considered an attempt to cheat on the exams and will result in a 0 on the grade. Test questions will be taken from material covered in lecture, assigned reading, and suggested problems. Exams, including the final exam, will be computer graded. It is the responsibility of the student to have a clean, flat, pink Test form (Scantron) with UCF logo, and a number 2 pencil for each exam and quiz. Students without the test form will not be allowed to take the exam. Make-up exam will be only given to students who missed an exam due to university-related businesses such as representing the university in a conference or an athletic team and jury duty call. Students requesting make-up exams must bring complete original documents for instructor’s consideration. The instructor reserves the right to modify the schedule, the testing procedure, and the grading basis if, in the professional judgment of instructor, such modification is in the best interest of fulfilling the course objectives, and assuring the academic integrity of the course and the institution. Success in CHM 2045 * Do not lobby/negotiate for a grade! * Students who attend classes and work consistently typically do very well in the course. So, get to every lecture and discussion session with Supplemental Instruction (SI) leader on time, concentrate, and pay attention to the material being covered! * UNDERSTANDING the various concepts is vital to learn chemistry. Memorizing is a recipe for disaster! * Review lecture material early and often. Do not wait until the last few minutes before a test to do the necessary revision. * Review the worked exercises/examples in the textbook. Also at the end of each chapter is a list of chapter goals. Those serve as helpful review tools. Find time to work on the suggested end-of-chapter problems. Practice makes perfection. * The instructor strongly encourages you to use office hours for discussing the material covered in classes and reviewing exams.

Get assistance ASAP, if needed. Please make use of the SI leader sessions and the Student Academic Resource Center (SARC); Howard Phillips Hall 113; www.sarc.sdes.ucf.edu. Honesty: Complete academic honesty is expected on all aspects of the course. Any unethical conduct will be fully prosecuted according to Florida law and university regulations. Please consult the current Undergraduate Catalog and/or The Golden Rule for definitions and policies. Student Disability Please supply appropriate documentation and meet with the Student Accessibility Services of UCF, at Ferrell Commons 7F Room 185, to discuss accommodations if required. All faculty members of UCF are required to document students' academic activity at the beginning of each course. In order to document that we began this course, I have added the following academic activity to be completed by the end of the first week of classes: A syllabus quiz will be given through Webcourses. CHM 2045C.0001

Week 1: Aug 26 - 30 2: Sept 2 – 6

Class Schedule COMPETENCIES Matter, Measurements, Units Chapter 1 textbook Matter, Measurements, and Units / Atoms, Elements, Ions Chapters 1-2

(no class Sept 2) 3: Sept 9 - 13 4: Sept 16 - 20 5: Sept 23 - 27 6: Sept 30 -Oct 4 7: Oct 7 - 11

Quiz 1 Atoms, Elements, Ions / Molecules, Compounds Chapters 2-3 Quiz 2 Molecules, Compounds Chapter 3 Test 1 Chemical Quantities & Aqueous Reactions Chapter 4 Quiz 3 Chemical Quantities & Aqueous Reactions Chapter 4 Quiz 4 Chemical Quantities & Aqueous Reactions / Thermochemistry Chapt. 4-6

8: Oct 14 - 18 9: Oct 21 -25 10: Oct 28 – Nov 1 11: Nov 4 - 8 12: Nov 11 - 15 13: Nov 18 – 22 14: Nov 25 – Dec 1 15: Friday Dec 6

Test 2 Thermochemistry / Atomic Structure Chapt. 6-7 Quiz 5 Atomic Structure / Electron Configuration and Periodicity Chapt.7-8 Quiz 6 Electron Configuration and Periodicity Chapt.8 Test 3 Chemical Bonding Part I Chapt. 9 Quiz 7 Chemical Bonding Part I / Chemical Bonding Part II Chapt. 9-10 Quiz 8 Chemical Bonding Part II Chapt.10 Test 4 Gases (no class Nov 27-29) Chapter 5 FINAL EXAM VAB – 132 7am to 9:50am

Holidays : Labor Day, Mon Sept 02 Veteran’s Day, Monday. Nov.11, Withdrawal Deadline: Friday, November 1, 2019

Thanksgiving, Nov 27 – 29....